Transcript Chemistry: Atoms First, McMurry and Fay, 1st Edition

John E. McMurry • Robert C. Fay
General Chemistry: Atoms First
Chapter 7
Reactions in Aqueous Solution
Lecture Notes
Alan D. Earhart
Southeast Community College • Lincoln, NE
Copyright © 2010 Pearson Prentice Hall, Inc.
Some Ways That Chemical
Reactions Occur
Precipitation Reactions: Processes in which soluble
ionic reactants yield an insoluble solid product that
falls out of solution.
Pb(NO3)2(aq) + 2KI(aq)
2KNO3(aq) + PbI2(s)
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Chapter 7/2
Some Ways That Chemical
Reactions Occur
Acid-Base Neutralization Reactions: Processes in
which an acid reacts with a base to yield water plus an
ionic compound called a salt.
HCl(aq) + NaOH(aq)
H2O(l) + NaCl(aq)
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Chapter 7/3
Some Ways That Chemical
Reactions Occur
Oxidation-Reduction (Redox) Reactions: Processes
in which one or more electrons are transferred
between reaction partners (atoms, molecules, or ions).
Mg(s) + 2HCl(aq)
MgCl2(aq) + H2(g)
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Chapter 7/4
Electrolytes in Aqueous
Solution
Electrolytes: Substances which dissolve in water to
produce conducting solutions of ions.
H 2O
Na1+(aq) + Cl1-(aq)
NaCl(s)
Nonelectrolytes: Substances which do not produce
ions in aqueous solutions.
H 2O
C12H22O11(s)
C12H22O11(aq)
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Chapter 7/5
Electrolytes in Aqueous
Solution
Strong Electrolytes: Compounds that dissociate to a
large extent into ions when dissolved in water.
H 2O
HCl(g)
H1+(aq) + Cl1-(aq)
Weak Electrolytes: Compounds that dissociate to a
small extent into ions when dissolved in water.
CH3CO2H(aq)
H1+(aq) + CH3CO21-(aq)
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Chapter 7/7
Electrolytes in Aqueous
Solution
Strong Acids: hydrochloric acid, hydrobromic acid,
hydroiodic acid, perchloric acid, nitric acid, sulfuric acid.
Electrolytes in Aqueous
Solution
Ionic compounds
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Chapter 7/9
Electrolytes in Aqueous
Solution
Weak acids
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Chapter 7/10
Electrolytes in Aqueous
Solution
Molecular compounds (other than any strong or weak
Chapter 7/11
electrolytes)
Electrolytes in Aqueous
Solution
Dissociation Equations
H 2O
2Na1+(aq) + SO42-(aq)
Na2SO4(s)
H 2O
FeBr3(s)
Fe3+(aq) + 3Br1-(aq)
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Chapter 7/12
Aqueous Reactions and Net
Ionic Equations
Molecular Equation: All substances in the chemical
equation are written using their complete formulas as
if they were molecules.
Pb(NO3)2(aq) + 2KI(aq)
2KNO3(aq) + PbI2(s)
strong electrolytes
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precipitate
Chapter 7/13
Aqueous Reactions and Net
Ionic Equations
Ionic Equation: All of the strong electrolytes are
written as ions.
Pb(NO3)2(aq)
2KI(aq)
Pb2+(aq) + 2NO31- (aq) + 2K1+(aq) + 2I1-(aq)
2K1+(aq) + 2NO31- (aq) + PbI2(s)
2KNO3(aq)
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Chapter 7/14
Aqueous Reactions and Net
Ionic Equations
Spectator Ions: Ions that undergo no change during
the reaction and appear on both sides of the reaction
arrow.
Pb2+(aq) + 2NO31- (aq) + 2K1+(aq) + 2I1-(aq)
2K1+(aq) + 2NO31- (aq) + PbI2(s)
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Chapter 7/15
Aqueous Reactions and Net
Ionic Equations
Net Ionic Equation: Only the ions undergoing change
are shown.
Pb2+(aq) + 2I1-(aq)
PbI2(s)
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Chapter 7/16
Precipitation Reactions and
Solubility Guidelines
Solubility: States how much of a compound will
dissolve in a given amount of solvent at a given
temperature.
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Chapter 7/17
Precipitation Reactions and
Solubility Guidelines
1. A compound is probably soluble if it contains one of
the following cations:
• Group 1A cation: Li1+, Na1+, K1+, Cs1+
• Ammonium ion: NH41+
2. A compound is probably soluble if it contains one of
the following anions:
• Halide: Cl1-, Br1-, I1• except Ag1+, Hg22+, and Pb2+ compounds
• Nitrate (NO31-), perchlorate (ClO41-), acetate (CH3CO21-),
sulfate (SO42-)
• except Ba2+, Hg22+, and Pb2+ sulfates
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Chapter 7/18
Precipitation Reactions and
Solubility Guidelines
Write the molecular, ionic, and net ionic equations for
the reaction that occurs when aqueous solutions of
AgNO3 and Na2CO3 are mixed.
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Chapter 7/19
Precipitation Reactions and
Solubility Guidelines
Write the molecular, ionic, and net ionic equations for
the reaction that occurs when aqueous solutions of
AgNO3 and Na2CO3 are mixed.
1. Write the chemical formulas of the products (use
proper ionic rules).
AgNO3(aq) + Na2CO3(aq)
AB + CD
Ag2CO3
+ NaNO3
CB + AD
double replacement reaction
Chapter 7/20
Precipitation Reactions and
Solubility Guidelines
Write the molecular, ionic, and net ionic equations for
the reaction that occurs when aqueous solutions of
AgNO3 and Na2CO3 are mixed.
2. Molecular Equation: Balance the equation and
predict the solubility of each possible product.
2AgNO3(aq) + Na2CO3(aq)
Ag2CO3(s) + 2NaNO3(aq)
Neither the cation nor the
anion is in the solubility list.
Contains a group 1A cation.
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Chapter 7/21
Precipitation Reactions and
Solubility Guidelines
Write the molecular, ionic, and net ionic equations for
the reaction that occurs when aqueous solutions of
AgNO3 and Na2CO3 are mixed.
3. Ionic Equation: Dissociate the soluble ionic
compounds.
2AgNO3(aq)
Na2CO3(aq)
2Ag1+(aq) + 2NO31- (aq) + 2Na1+(aq) + CO32-(aq)
Ag2CO3(s) + 2Na1+(aq) + 2NO31-(aq)
2NaNO3(aq)
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Chapter 7/22
Precipitation Reactions and
Solubility Guidelines
Write the molecular, ionic, and net ionic equations for
the reaction that occurs when aqueous solutions of
AgNO3 and Na2CO3 are mixed.
4. Net Ionic Equation: Eliminate the spectator ions from
the ionic equation.
2Ag1+(aq) + 2NO31- (aq) + 2Na1+(aq) + CO32-(aq)
Ag2CO3(s) + 2Na1+(aq) + 2NO31-(aq)
2Ag1+(aq) + CO32-(aq)
Ag2CO3(s)
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Chapter 7/23
Acids, Bases, and
Neutralization Reactions
Acid (Arrhenius): A substance that dissociates in
water to produce hydrogen ions, H1+:
HA(aq)
H1+(aq) + A1-(aq)
HCl(aq)
H1+(aq) + Cl1-(aq)
In water, acids produce hydronium ions, H3O1+:
HCl(aq) + H2O(aq)
H3O1+(aq) + Cl1-(aq)
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Chapter 7/24
Acids, Bases, and
Neutralization Reactions
Base (Arrhenius): A substance that dissociates in
water to produce hydroxide ions, OH1-:
MOH(aq)
M1+(aq) + OH1-(aq)
NaOH(aq)
Na1+(aq) + OH1-(aq)
Ammonia, commonly called “ammonium hydroxide” is
a base:
NH3(aq) + H2O(aq)
NH41+(aq) + OH1-(aq)
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Chapter 7/25
Acids, Bases, and
Neutralization Reactions
Strong acids and strong bases are strong electrolytes.
Weak acids and weak bases are weak electrolytes.
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Chapter 7/26
“ous”
“ic”
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“ite”
“ate”
Chapter 7/27
Acids, Bases, and
Neutralization Reactions
Binary Acids
HCl
hydrochloric acid
HBr
hydrobromic acid
HF
hydrofluoric acid
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Chapter 7/28
Acids, Bases, and
Neutralization Reactions
These acid-base neutralization reactions are doublereplacement reactions just like the precipitation
reactions:
HA + MOH
MA + HOH
or
HA + MOH
Acid
Base
MA + H2O
Salt
Water
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Chapter 7/29
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous HBr and aqueous Ba(OH)2.
1. Write the chemical formulas of the products (use
proper ionic rules for the salt).
HBr(aq) + Ba(OH)2(aq)
Acid
Base
H2O
+ BaBr2
Water
Salt
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Chapter 7/30
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous HBr and aqueous Ba(OH)2.
2. Molecular Equation: Balance the equation and
predict the solubility of the salt in the products.
2HBr(aq) + Ba(OH)2(aq)
2H2O(l) + BaBr2(aq)
Use the solubility rules.
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Chapter 7/31
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous HBr and aqueous Ba(OH)2.
3. Ionic Equation: Dissociate a strong acid and the
soluble ionic compounds.
2HBr(aq)
Ba(OH)2(aq)
2H1+(aq) + 2Br1-(aq) + Ba2+(aq) + 2OH1-(aq)
2H2O(l) + Ba2+(aq) + 2Br1-(aq)
BaBr2(aq)
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Chapter 7/32
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous HBr and aqueous Ba(OH)2.
4. Net Ionic Equation: Eliminate the spectator ions from
the ionic equation.
2H1+(aq) + 2Br1-(aq) + Ba2+(aq) + 2OH1-(aq)
2H2O(l) + Ba2+(aq) + 2Br1-(aq)
2H1+(aq) + 2OH1-(aq)
or
H1+(aq) + OH1-(aq)
2H2O(l)
H2O(l)
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Chapter 7/33
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous NaOH and aqueous HF.
1. Write the chemical formulas of the products (use
proper ionic rules for the salt).
HF(aq) + NaOH(aq)
Acid
Base
H2O
Water
+ NaF
Salt
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Chapter 7/34
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous NaOH and aqueous HF.
2. Molecular Equation: Balance the equation and
predict the solubility of the salt in the products.
HF(aq) + NaOH(aq)
H2O(l) + NaF(aq)
Use the solubility rules.
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Chapter 7/35
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous NaOH and aqueous HF.
3. Ionic Equation: Dissociate a strong acid and the
soluble ionic compounds.
NaOH(aq)
HF(aq) + Na1+(aq) + OH1-(aq)
H2O(l) + Na1+(aq) + F1-(aq)
NaF(aq)
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Chapter 7/36
Acids, Bases, and
Neutralization Reactions
Write the molecular, ionic, and net ionic equations for
the reaction of aqueous NaOH and aqueous HF.
4. Net Ionic Equation: Eliminate the spectator ions from
the ionic equation.
HF(aq) + Na1+(aq) + OH1-(aq)
HF(aq) + OH1-(aq)
H2O(l) + Na1+(aq) + F1-(aq)
H2O(l) + F1-(aq)
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Chapter 7/37
Chapter 7/38
Oxidation-Reduction (Redox)
Reactions
4Fe(s) + 3O2(g)
2Fe2O3(s) + 3C(s)
2Fe2O3(s)
4Fe(s) + 3CO2(g)
Rusting of iron:
an oxidation of Fe
Manufacture of iron:
a reduction of Fe
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Chapter 7/39
Oxidation-Reduction (Redox)
Reactions
Oxidation: The loss of one or more electrons by a
substance, whether element, compound, or ion.
Reduction: The gain of one or more electrons by a
substance, whether element, compound, or ion.
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Chapter 7/40
Oxidation-Reduction (Redox)
Reactions
Oxidation Number (State): A value which indicates
whether an atom is neutral, electron-rich, or electronpoor.
Rules for Assigning Oxidation Numbers
1. An atom in its elemental state has an oxidation
number of 0.
Na
H2
Br2
S
Ne
Oxidation number 0
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Chapter 7/41
Oxidation-Reduction (Redox)
Reactions
2. An atom in a monatomic ion has an oxidation
number identical to its charge.
Na1+
Ca2+
Al3+
Cl1-
O2-
+1
+2
+3
-1
-2
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Chapter 7/42
Oxidation-Reduction (Redox)
Reactions
3. An atom in a polyatomic ion or in a molecular
compound usually has the same oxidation number
it would have if it were a monatomic ion.
a) Hydrogen can be either +1 or -1.
1-
H
O
+1
-2
H
Ca H
-1
+2
-1
b) Oxygen usually has an oxidation number of -2.
H
+1
O
-2
H
+1
H
+1
O
-1
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O
-1
H
+1
Chapter 7/43
Oxidation-Reduction (Redox)
Reactions
3.
c) Halogens usually have an oxidation number of -1.
H
Cl
+1
-1
Cl
+1
O
-2
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Cl
+1
Chapter 7/44
Oxidation-Reduction (Redox)
Reactions
4. The sum of the oxidation numbers is 0 for a neutral
compound and is equal to the net charge for a
polyatomic ion.
H2SO3
+1
x
-2
Cr2O72x
-2
2(+1) + x + 3(-2) = 0 (net charge)
x = +4
2(x) + 7(-2) = -2 (net charge)
x = +6
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Chapter 7/45
Identifying Redox Reactions
Reducing Agent
•
•
•
•
Causes reduction
Loses one or more electrons
Undergoes oxidation
Oxidation number of atom increases
Oxidizing Agent
•
•
•
•
Causes oxidation
Gains one or more electrons
Undergoes reduction
Oxidation number of atom decreases
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Chapter 7/46
Identifying Redox Reactions
Reducing Agent
oxidation
0
+3
4Fe(s) + 3O2(g)
2Fe2O3(s)
0
Oxidizing Agent
-2
reduction
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Chapter 7/47
Identifying Redox Reactions
Reducing Agent
oxidation
0
2Fe2O3(s) + 3C(s)
+3
Oxidizing Agent
+4
4Fe(s) + 3CO2(g)
-2
reduction
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Chapter 7/48
The Activity Series of the
Elements
Cu(s) + 2Ag1+(g)
Cu2+(aq) + 2Ag(s)
Which one of these reactions will occur?
2Ag(s) + Cu2+(g)
2Ag1+(aq) + Cu(s)
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Chapter 7/49
The Activity Series of the
Elements
The elements that are
higher up in the table
are more likely to be
oxidized.
Thus, any element
higher in the activity
series will reduce the
ion of any element
lower in the activity
series.
Chapter 7/50
Balancing Redox Reactions:
The Half-Reaction Method
Balancing Redox Reactions:
The Half-Reaction Method
Balance the following net ionic equation in acidic
solution:
I1-(aq) + Cr2O72-(aq)
Cr3+(aq) + IO31-(aq)
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Chapter 7/53
Balancing Redox Reactions:
The Half-Reaction Method
•
Write the two unbalanced half-reactions.
Cr2O72-(aq)
I1-(aq)
Cr3+(aq)
IO31-(aq)
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Chapter 7/54
Balancing Redox Reactions:
The Half-Reaction Method
•
Multiply each half-reaction by a factor to make the
electron count the same in both half-reactions.
reduction: 14H1+(aq) + Cr2O72-(aq)
oxidation:
6e- + 3H2O(l) + I1-(aq)
2Cr3+(aq) + 7H2O(l) + 6eIO31-(aq) + 6H1+(aq)
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Chapter 7/55
Balancing Redox Reactions:
The Half-Reaction Method
•
Add the two balanced half-reactions together and
cancel species that appear on both sides of the
equation.
reduction: 14H1+(aq) + Cr2O72-(aq)
2Cr3+(aq) + 7H2O(l) + 6eoxidation:
6e- + 3H2O(l) + I1-(aq)
IO31-(aq) + 6H1+(aq)
8H1+(aq) + I1-(aq) + Cr2O72-(aq)
IO31-(aq) + 2Cr3+(aq) + 4H2O(l)
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Chapter 7/56
Balancing Redox Reactions:
The Half-Reaction Method
Balance the following net ionic equation in basic
solution:
MnO41-(aq) + Br1-(aq)
MnO2(s) + BrO31-(aq)
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Chapter 7/57
Balancing Redox Reactions:
The Half-Reaction Method
•
Write the two unbalanced half-reactions.
Br1-(aq)
MnO41-(aq)
BrO31-(aq)
MnO2(s)
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Chapter 7/58
Balancing Redox Reactions:
The Half-Reaction Method
•
Balance both half-reactions for all atoms except O and
H.
Br1-(aq)
MnO41-(aq)
BrO31-(aq)
MnO2(s)
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Chapter 7/59
Balancing Redox Reactions:
The Half-Reaction Method
•
Balance each half-reaction for O by adding H2O, and
then balance for H by adding H1+.
3H2O(l) + Br1-(aq)
4H1+(aq) + MnO41-(aq)
BrO31-(aq) + 6H1+(aq)
MnO2(s) + 2H2O(l)
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Chapter 7/60
Balancing Redox Reactions:
The Half-Reaction Method
•
Balance each half-reaction for charge by adding
electrons to the side with greater positive charge.
3H2O(l) + Br1-(aq)
3e- + 4H1+(aq) + MnO41-(aq)
BrO31-(aq) + 6H1+(aq) + 6eMnO2(s) + 2H2O(l)
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Chapter 7/61
Balancing Redox Reactions:
The Half-Reaction Method
•
Multiply each half-reaction by a factor to make the
electron count the same in both half-reactions.
3H2O(l) + Br1-(aq)
2 3e- + 4H1+(aq) + MnO41-(aq)
BrO31-(aq) + 6H1+(aq) + 6eMnO2(s) + 2H2O(l)
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Chapter 7/62
Balancing Redox Reactions:
The Half-Reaction Method
•
Add the two balanced half-reactions together and
cancel species that appear on both sides of the
equation.
3H2O(l) + Br1-(aq)
BrO31-(aq) + 6H1+(aq) + 6e-
6e- + 8H1+(aq) + 2MnO41-(aq)
2MnO2(s) + 4H2O(l)
2H1+(aq) + 2MnO41-(aq) + Br1-(aq)
2MnO2(s) + H2O(l) + BrO31-(aq)
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Chapter 7/63
Balancing Redox Reactions:
The Half-Reaction Method
•
Since the reaction occurs in a basic solution,
“neutralize” the excess H1+ by adding OH1- and cancel
any water (if possible).
2H2O
2OH1-(aq) + 2H1+(aq) + 2MnO41-(aq) + Br1-(aq)
2MnO2(s) + H2O(l) + BrO31-(aq) + 2OH1-(aq)
H2O(l) + 2MnO41-(aq) + Br1-(aq)
2MnO2(s) + BrO31-(aq) + 2OH1-(aq)
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Chapter 7/64
Redox Stoichiometry
Titration: A procedure for determining the concentration
of a solution by allowing a carefully measured volume to
react with a solution of another substance (the standard
solution) whose concentration is known.
5H2C2O4(aq) + 2MnO41-(aq) + 6H1+(aq)
10CO2(g) + 2Mn2+(aq) + 8H2O(l)
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Chapter 7/65
Chapter 7/66
Redox Stoichiometry
A solution is prepared with 0.2585 g of oxalic acid,
H2C2O4. 22.35 mL of an unknown solution of potassium
permanganate are needed to titrate the solution. What is
the concentration of the potassium permanganate
solution?
5H2C2O4(aq) + 2MnO41-(aq) + 6H1+(aq)
10CO2(g) + 2Mn2+(aq) + 8H2O(l)
Mass of
H2C2O4
Moles of
H2C2O4
Molar Mass
of H2C2O4
Moles of
KMnO4
Mole Ratio
Molarity of
KMnO4
Molarity of
KMnO4
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Chapter 7/67
Redox Stoichiometry
5H2C2O4(aq) + 2MnO41-(aq) + 6H1+(aq)
10CO2(g) + 2Mn2+(aq) + 8H2O(l)
Moles of H2C2O4 available:
0.2585 g H2C2O4
x
1 mol
90.04 g
= 0.002871 mol H2C2O4
Moles of KMnO4 reacted:
0.002871 mol H2C2O4 2 mol KMnO4
x
= 0.001148 mol KMnO4
5 mol H2C2O4
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Chapter 7/68
Redox Stoichiometry
5H2C2O4(aq) + 2MnO41-(aq) + 6H1+(aq)
10CO2(g) + 2Mn2+(aq) + 8H2O(l)
Concentration of KMnO4 solution:
0.001148 mol KMnO4
22.35 mL
1000 mL
x
1L
= 0.05136 M KMnO4
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Chapter 7/69